For the following reaction,CO(g)H₂O(g) →CO₂ (9)a. Write the Kc expression for this reaction.b. If a 1.00L vessel is charged with 0.250 moles of CO, 0.250 moles of H₂0, 0.750 males of CO₂, and 0.750 males of H₂, what is the value of Q?+ H₂ (9)Kc = 1.845c. In which direction does the reaction progress to establish equilibrium?d. What are the equilibrium concentration of all species?

Answer: Given chemical reaction: CO(g)+H2O(g)⇌CO2(g)+H2(g) Kc=1.845

For the following reaction, co (g) - H₂O(g) →CO₂(g) + H₂ (0) Kc = 1.845 a. While the Ko expression for this reaction. b. If a 1.00L vessel is charged with 0.250 moles of CO, 0.250 moles of H₂0, 0.750 moles of CO₂, and 0.750 moles of H₂, what is the value of Q? c. In which direction does the reaction progress to establish equilibrium? d. What are the equilibrium concentration of all species?

For the following reaction, co (g) - H₂O(g) →CO₂(g) + H₂ (0) Kc = 1.845 a. While the Ko expression for this reaction. b. If a 1.00L vessel is charged with 0.250 moles of CO, 0.250 moles of H₂0, 0.750 moles of CO₂, and 0.750 moles of H₂, what is the value of Q? c. In which direction does the reaction progress to establish equilibrium? d. What are the equilibrium concentration of all species?

Chemistry & Chemical Reactivity

10th Edition

ISBN:9781337399074

Author:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Publisher:John C. Kotz, Paul M. Treichel, John Townsend, David Treichel

Chapter5: Principles Of Chemical Reactivity: Energy And Chemical Reactions

Section5.8: Product- Or Reactant-favored Reactions And Thermodynamics

Problem 2.1ACP

See similar textbooks

Similar questions

Calculate H when a 38-g sample of glucose, C6H12O6(s), burns in excess O2(g) to form CO2(g) and H2O() in a reaction at constant pressure and 298.15 K.
Use the appropriate tables to calculate H for (a) the reaction between copper(II) oxide and carbon monoxide to give copper metal and carbon dioxide. (b) the decomposition of one mole of methyl alcohol (CH3OH) to methane and oxygen gases.
When 7.11 g NH4NO3 is added to 100 mL water, the temperature of the calorimeter contents decreases from 22.1 C to 17.1 C. Assuming that the mixture has the same specific heat as water and a mass of 107 g, calculate the heat q. Is the dissolution of ammonium nitrate exothermic or endothermic?
One of the components of polluted air is NO. It is formed in the high-temperature environment of internal combustion engines by the following reaction: N2(g)+O2(g)2NO(g)H=180KJ Why are high temperatures needed to convert N2 and O2 to NO?
8. A hydrocarbon fuel is fully combusted with 495.97 g of oxygen to yield 880.2 g of carbon dioxide and 396.34 g of water. A.) Find the empirical formula for the hydrocarbon. B.) The molecular formula of the hydrocarbon if its MW is 142.29 g/mol. 9. (5 points) The K, value of the reaction N₂O4 2NO₁₂ (g) ²(g) is 0.113. What is the Gibbs free energy, AG, of the reaction if the initial pressure of N₂O4 is 1.23 atm while NO₂ is 0.750 atm? Is the process spontaneous? 10. (5 points) The molar heat of vaporization of ammonia is 23.4 kJ/mol while its boiling point is -33.34 °C. Calculate the AS for the vaporization of 0.75 moles of ammonia. Express your answer with unit J/K.
what is delta Hr for the reaction 3NH3 (g) + 3.75 (g) - 3NO(g) + 4.5 H20 (g) delta Hr = -904.7KJ 4NH3 (g) + 5O (g) ----> 4NO(g) + 6 H20 (g) delta Hr= -904.7 JK
Consider the balanced reaction 4 A + 4 B → 5C+ 6 D. If 5.577 moles of C (MW = 36.53) are produced, how many grams of A (MW%3D 47.16) are consumed? Report your answer to three decimal places (ignore significant figures).
18. For the following combustion reaction of benzoic acid (HC¬H5O2; molar mass = 122.1 g/mol) HC;H5O2(s) + 15202(g) --> 7CO2(g) + 3H20(1); DHcomb = -3226 kJ 1.00 g of benzoic acid is combusted in a bomb calorimeter, which contains 1.00 kg of water (specific heat = 4.184 J/g.°C) and the bomb has a heat capacity of 890 J/°C. If the initial temperature of the calorimeter is 25.0°C, what is the final temperature of the calorimeter when the combustion is completed? (A) 51.8°C (B) 31.3°C (C) 30.2°C (D) 27.0°C
4. The reaction of HCl(aq) and NaOH(aq) is exothermic. The equation is : HСI (аq) + NaОН (аq) NaC (аq) + H20(1) In one experiment 50.0 mL of 1.00M HCl at 25.50 °C was placed in a calorimeter. To this 50.00 mL of 1.0o M NaOH at 25.50 °C was added. The mixture was stirred and the temperature rose to coffee cup 32.40 °C. What is the energy evolved in joules per mole of HCl, CH20 = 4.184 jg1ºCª. SHOW ALL YOUR WORK. -10
(1) two baking sheets are made of different metals. you purchase both and bake a dozen cookies on each sheet at the same time in your oven. you observe that after 9 minutes, the cookies on one sheet are slightly burned on the bottom, whereas those on the other sheet are fine. (you are curious and you vary the conditions so you know the result is not caused by the oven.) (a) how can you use this observation to infer something about the specific heat of the materials in the baking sheets? (b) what is the mathematical reasoning (equation) that you need to support your conclusion?
(Q77) The standard Gibbs free energy (AG°rxn) for the formation of sulfur trioxide from sulfur dioxide and oxygen gas is -72.3 kJ/mol. The balanced chemical equation is SO2 (g) + ½ O2 (g) --> SO3 (g). What will be the Gibbs Free energy of the reaction (in kJ/mol) if it takes place at a low temperature of -13.7 and the concentrations of three gases are: SO2 = 0.112 M %3D O2 = 0.110 M SO3 = 1.74 M
What is true for this chemical reaction:: 4FeS₂ (s) + 150₂(g) + 8H₂O(1) a Select an answer and submit. For keyboard navigation, use the up/down arrow keys to select an answer. b с d AHrxn > 0; ASrxn 0 - AHrxn > 0; ASrxn > 0 2Fe₂O3(s) + 8H₂SO4 (aq)?